Barium nitrite

The names adopted for salts consisted of a generic part derived from the acid and a specific part from the metallic base r oxide de plomb + I acide sulfurique le sulfate de plomb. The names for salts of acids containing an element in different degrees of oxidation were given different terminations sufte de soude and sulfate de soude for sodium sulfite and sulfate, and nitrite de baryte and nitrate de baryte for barium nitrite and nitrate. 

Ammonium nitrite [13446-48-5] NH4NO2, a compound of questionable stabiUty, can be prepared by reaction of barium nitrite and aqueous ammonium sulfate. After removal of the precipitated barium sulfate by filtration, the ammonium nitrite can be recovered from solution. The salt is said to decompose, sometimes explosively, at 60—70°C. 

Silver Nitrite. Silver nitrite, AgN02, is prepared from silver nitrate and a soluble nitrite, or silver sulfate and barium nitrite. 

Barium nitrite [13465-94-6] Ba(N02)2, crystallines from aqueous solution as barium nitrite monohydrate [7787-38-4], Ba(N02)2 H2O, which has yellowish hexagonal crystals, sp gr 3.173, solubihty 54.8 g Ba(NO2)2/100 g H2O at 0°C, 319 g at 100°C. The monohydrate loses its water of crystallization at 116°C. Anhydrous barium nitrite, sp gr 3.234, melts at 267°C and decomposes at 270 °C into BaO, NO, and N2. Barium nitrite may be prepared by crystallization from a solution of equivalent quantities of barium chloride and sodium nitrite, by thermal decomposition of barium nitrate in an atmosphere of NO, or by treating barium hydroxide or barium carbonate with the gaseous oxidiation products of ammonia. It has been used in diazotization reactions. 

The Deamination of Adenosine 20 g of adenosine are dissolved in one liter of water by warming, and after cooling to room temperature 120 g of barium nitrite (monohydrate) are added to the solution. Under stirring there is added in time intervals of one hour 160 cc of 2N sulfuric acid after each time interval. After the third addition, the reaction mass is allowed to stand for 3 hours at room temperature. The solution is then tested for barium, and if some barium is still present a slight excess of sulfuric acid is added. 300 cc of methanol is then added. In order to drive off the excess of nitrous acid, CO is conducted... 

Barbituric acid Minoxidil Barium hydroxide Cyclobutyroi Barium nitrite I nosine... 

In an atmosphere of nitric oxide, thermal decomposition produces barium nitrite, Ba(N02)2. Reactions with soluble metal sulfates or sulfuric acid yield barium sulfate. Many insoluble barium salts, such as the carbonate, oxalate and phosphate of the metal, are precipitated by similar double decomposition reactions. Ba(N03)2 is an oxidizer and reacts vigorously with common reducing agents. The solid powder, when mixed with many other metals such as aluminum or zinc in their finely divided form, or combined with alloys such as... 

Hydrazine (or Hydrazinium) Nitrite. N2H4.HNO2 mw 79.06, N 53.15% decomp or explodes on rapid heating colorless to yellowish hygr solid sol in w ale insol in eth may be prepd by mixing solns of barium nitrite and neutral hydrazine sulfate, as described in Mellor (Ref 1). Explodes violently on impact and less so when rapidly heated. When heated slowly it decomposes according to the equation ... 

Nitro-pentammino-cobaltic Nitrite, [Co(NH3)5(N02)](N02)2. 2H20, is prepared by heating aquo-pentammino-eobaltic sulphate with barium nitrite, or by treating a solution of chloro-pentammino-cobaltie 1 Werner, Ber., 1907, 40, 284. 

Barium nitrite (H2O) [7787-38-4] M 247.4. Crystd from water (Iml/g) by cooling in an ice-salt bath. 

It was prepared by Berzelius as early as 1812 [50] by treating lead nitrite with ammonium sulphate. Later M. Berthelot [50] obtained it by acting with barium nitrite on ammonium sulphate. Erdmann and Sorensen [50] prepared it by acting with dinitrogen tetroxide on coarsely ground ammonium carbonate near 0°C. Ammonium nitrite cannot be obtained from its aqueous solution, as it decomposes on evaporating. 

B. C. Dutt and S. N. Sen found that when nitric oxide is passed into a suspension of barium dioxide in water, barium nitrite, not nitrate, is formed. P. Sabatier and J. B. Senderens observed no change when nitric oxide is passed over Cuprous Oxide at 500°. H. A. Auden and G. J. Fowler observed that dry nitric oxide and Silver oxide, at ordinary temp., form silver and silver nitrate P. Sabatier and J. B. Senderens also obtained silver and silver nitrite by passing nitric oxide into water with silver oxide in suspension. C. F. Schonbein found gold oxide is reduced by moist nitric oxide, forming nitrous acid. P. Sabatier and J. B. Senderens found that titanium sesquioxide forms white titanic oxide when heated in an atm. of nitric oxide and that stannous oxide below 500° burns in an atm. of nitric oxide, forming stannic oxide. If nitric oxide be passed into water with lead dioxide in suspension, the water is coloured, and in about 3 hrs., lead nitrite and nitrate are formed, and later, rhombic crystals of a basic nitrite. B. C. Dutt and S. N. Sen said that the nitrate is formed by the action of the dioxide on the nitrite. Lead dioxide is reduced to lead oxide by nitric oxide at 315°, and H. A. Auden and G. J. Fowler found that the reaction begins at 15°, when a basic lead nitrite is... 

The same salt was prepared by E. Peligot by adding barium nitrite to a soln. of silver nitrate. E. Mitsoherlioh, and V. Kohlschiitter and E. Eydmann added sodium nitrite to a soln. of silver nitrate, and crystallized the precipitated silver nitrite (and oxide) from its soln. in boiling water V. Meyer worked with potassium nitrite and silver nitrate J. Persoz melted equal parts of silver and potassium nitrates, and crystallized the silver nitrite from hot water. E. Priwoznik treated an excess of silver with nitric acid W. J. Russell, and A. R. Leeds passed hydrogen into a cone. soln. of silver nitrate and E. Divers heated silver nitrate in a current of nitric oxide. The aq. soln. decomposes below 100°, and J. Lang, and N. W. Fischer said that the losses are so great when the attempt is made to purify the salt by recrystallization, that it is better instead to wash the salt with a little cold water. A. Naumann and A. Rucker crystallized the salt from a soln. of nitrous acid. 

W. Meyerhofler said that under the conditions here described, the salt pair, barium nitrite and sodium chloride, is stable within its interval of change, and that in the presence of water it will separate as a third salt, while barium chloride and sodium nitrite will remain in soln. To prevent this an excess of sodium nitrite is necessary. J. Matuschek showed that hydrated barium chloride and sodium nitrite, interact when pounded together, and that these salts react in molecular proportion in aq. soln. at 100° if only a limited amount of water is present. The yield of barium nitrite approaches the theoretical when the amount of water added as solvent is one-third of the weight of the nitrite which would be formed if the reaction were quantitative. 

Fig. 82.—Solubility Fig. 83.—Solu- Fig. 84.—Solubility of Calcium Nitrite. bility of Stron- of Barium Nitrite, tium Nitrite.

At higher temp., the salt is much hydrolyzed. W. Hampe, and J. Lang noted that strontium nitrate is very soluble in water, and P. Vogel found that 100 c.c. of a soln. at 19-5° has 62-83 grms. of Sr(N02)2.H20 while M. Oswald obtained the results indicated in Pig. 83. The eutectic at —6-8° has 32-8 per cent. Sr(N02)2. Por the solubility, S, of monohydrated strontium and barium nitrites, per 100 parts of water, M. Oswald gave ... 

P. 0. Ray and N. R. Dhar also measured the electrical conductivities of soln. of the three nitrites and P. C. Ray and 8. C. Mukherjee observed that the degrees of ionization of soln. of calcium nitrite at dilutions t =28-0 and 19-4 litres are respectively 0-84 and 0-82 for strontium nitrite at dilutions v—22-0 and 21-0 litres, 0-84 in both cases and for barium nitrite for c=21-0 and 31-4 litres, respectively 0-84 and 0-86. 

According to E. C. Franklin and C. A. Kraus, a soln. of barium nitrite in liquid ammonia reacts with the following salts dissolved in liquid ammonia—ammonium chloride, bromide, and iodide are precipitated ammonium chromate gives a... 

BaAg2(N02)4.H20, from a soln. of the component salts. The formula is here due to M. Oswald, who examined the three nitrites of the alkaline earths, and found only barium forms a double salt. The conditions of stability are represented by AB, Fig. 85. The corresponding diagrams for strontium and calcium nitrites do not show any evidence of the formation of silver strontium nitrite, or of a silver calcium nitrite nor is any strontium barium nitrite formed, for the two salts give a series of mixed crystals, (Ba,Sr)(N02)2.H20. 

F. Vogel tried without success to make beryllium nitrite by the action of beryllium sulphate on barium nitrite. He found that in aq. soln. the precipitate is immediately hydrolyzed, nitrogen oxides are evolved, and only a small proportion of nitrogen remains. It might be added that many salts, unstable in aq. soln., have... 

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